The following reaction is first order inN 2 O 5 : N 2 O 5 (g) -----> NO 3 (g) +

Question

The following reaction is first order inN2O5: N2O5 (g) -----> NO3(g) + NO2(g) The rate constand for the reaction at a certain temperature is0.053/s. Calculate the rate of reaction when[N2O5] = 5.2x10-2 M. Rate= _______ M/s Also, what would the rate of reaction be at the sameconcentration if the reaction were in second order? Rate = ______ M/s Zero order? Rate = ______ M/s thank you! :) The following reaction is first order inN2O5: N2O5 (g) -----> NO3(g) + NO2(g) The rate constand for the reaction at a certain temperature is0.053/s. Calculate the rate of reaction when[N2O5] = 5.2x10-2 M. Rate= _______ M/s Also, what would the rate of reaction be at the sameconcentration if the reaction were in second order? Rate = ______ M/s Zero order? Rate = ______ M/s thank you! :)

Explanation / Answer

N2O5 (g) -----> NO3(g) + NO2(g) Since the reaction is first order reaction the rate law isRate r = k [N2O5] Where k = rate constant = 0.053 / s          [ N2O5 ] =5.2 * 10^-2 M Plug the values we get r = 2.756*10^-3 M/s For a second order reaction Rate r' = k [N2O5]2                                                         = 0.053 /s * ( 5.2 * 10^-2 ) 2                                                         = 1.433 * 10^-4 M/s For Zero order reaction rate r'' = k = 0.053M/s                                                         = 1.433 * 10^-4 M/s For Zero order reaction rate r'' = k = 0.053M/s

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